Solutions and Colligative Properties - Result Question 54

####25. An organic compound (CxH2yOy) was burnt with twice the amount of oxygen needed for complete combustion to CO2 and H2O. The hot gases when cooled to 0C and 1atm pressure, measured 2.24L. The water collected during cooling weight 0.9g. The vapour pressure of pure water at 20C is 17.5mmHg and is lowered by 0.104mm when 50g of the organic compound are dissolved in 1000g of water. Give the molecular formula of the organic compound.

(1983,5M)

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Solution:

  1. From lowering of vapour pressure information :

0.10417.5=χ2=n2n1+n2 n1n2+1=168.27 n1n2=167.27 100018×M50=167.27 M=150g/mol

Also, the combustion reaction is :

CxH2yOy+xO2xCO2+yH2O

18yg of H2O is produced from 1.0 mole of compound.

0.9g of H2O will be produced from 0.918y=120y mol

At the end, moles of O2 left =x20y

moles of CO2 formed =x20y

Total moles of gases at STP =2x20y=2.2422.4

x=y

Molar mass; 150=12x+2x+16x=30x

x=15030=5

Formula =C5H10O5



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